Worksheet: Osmotic Concentration
In this worksheet, we will practice describing how dissociation affects osmosis and converting osmotic pressures to molar concentrations.
The osmotic pressure of human blood is 7.6 atm at . What mass of glucose, , is required to make 1.00 L of aqueous solution for intravenous feeding if the solution must have the same osmotic pressure as blood at body temperature, ?
A 0.010 M solution of the weak acid has an osmotic pressure of 0.293 atm at . A 0.010 M solution of the weak acid has an osmotic pressure of 0.345 atm under the same conditions. Each solution contains three dissolved species: the weak acid ( or ), the conjugate base ( or ), and the hydrogen ion (). The osmotic pressure of each solution is related to the solute concentrations in molar units.
Which acid has the larger equilibrium constant for ionization, or ?
What is the equilibrium constant for the ionization of ?